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प्रश्न
Explain the following:
Silica is added to the sulphide ore of copper in the reverberatory furnace.
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उत्तर
Copper pyrites contain iron sulphide in addition to copper sulphide. In the reverberatory furnace copper ore is roasted to give oxides. \[\ce{FeO}\] is removed by adding silica from the matte containing \[\ce{Cu2S}\] and \[\ce{FeS}\].
\[\ce{2FeS + 3O2 -> 2FeO + 2SO2}\]
\[\ce{Feo + SiO2 -> \underset{(Slag)}{FeSiO3}}\]
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संबंधित प्रश्न
Why is the extraction of copper from pyrites more difficult than that from its oxide ore through reduction?
Write down the reactions taking place in different zones in the blast furnace during the extraction of iron.
The choice of a reducing agent in a particular case depends on thermodynamic factor. How far do you agree with this statement? Support your opinion with two examples.
The impurity that is added externally to remove the impurity already present in the ore is known as ____________.
In the extraction of copper from its sulphide ore, the metal is formed by the reduction of \[\ce{Cu2O}\] with ______.
In the metallurgy of aluminium ______.
The purest form of iron is prepared by oxidising impurities from cast iron in a reverberatory furnace. Which iron ore is used to line the furnace? Explain by giving reaction.
The mixture of compounds A and B is passed through a column of \[\ce{Al2O3}\] by using alcohol as eluant. Compound A is eluted in preference to compound B. Which of the compounds A or B, is more readily adsorbed on the column?
Why is sulphide ore of copper heated in a furnace after mixing with silica?
Write down the reactions taking place in Blast furnace related to the metallurgy of iron in the temperature range 500-800 K.
Explain the following:
\[\ce{CO2}\] is a better reducing agent below 710 K whereas \[\ce{CO}\] is a better reducing agent above 710 K.
Explain the following:
Generally sulphide ores are converted into oxides before reduction.
Explain the following:
Carbon and hydrogen are not used as reducing agents at high temperatures.
Carbon deposition reaction taking place in ______.
\[\ce{Au + CN^- + H2O + O2 -> [Au(CN)2]^- + OH^-}\]
The number of CN− ions involved in the balanced equation is ______.
